When you break or crush an ionic compound, you are physically separating the individual ions that make up the compound. However, the chemical bonds between the ions remain intact, so the compound's chemical formula and properties are preserved. The compound may exhibit different physical properties, such as a change in shape or size, but its chemical composition remains the same.
Both acids and ionic compounds release ions in solution. Acids release H+ ions, while ionic compounds dissociate into cations and anions. This ionization allows both substances to conduct electricity in solution.
Ionic compounds are dissociated in water solution.
When ionic compounds dissolve in water, they dissociate into their constituent ions. These ions are surrounded by water molecules, which help stabilize them in solution. This process allows ionic compounds to conduct electricity in solution and is the basis for many chemical reactions.
Covalent compounds have lower melting points compared to ionic compounds because covalent bonds are generally weaker than ionic bonds. In covalent compounds, individual molecules or atoms are held together by shared electrons, which are weaker than the electrostatic attraction in ionic compounds. Hence, less energy is required to break the bonds in covalent compounds, resulting in lower melting points.
Ionic compounds generally have a higher volatility compared to covalent compounds. This is because ionic compounds have weaker intermolecular forces that allow them to break apart and vaporize more easily at lower temperatures. Covalent compounds tend to have stronger intermolecular forces, making them less likely to evaporate at the same rate.
Nothing, ionic compounds on cooling remain as they were.
Both acids and ionic compounds release ions in solution. Acids release H+ ions, while ionic compounds dissociate into cations and anions. This ionization allows both substances to conduct electricity in solution.
Ionic compounds are dissociated in water solution.
When ionic compounds dissolve in water, they dissociate into their constituent ions. These ions are surrounded by water molecules, which help stabilize them in solution. This process allows ionic compounds to conduct electricity in solution and is the basis for many chemical reactions.
Covalent compounds have lower melting points compared to ionic compounds because covalent bonds are generally weaker than ionic bonds. In covalent compounds, individual molecules or atoms are held together by shared electrons, which are weaker than the electrostatic attraction in ionic compounds. Hence, less energy is required to break the bonds in covalent compounds, resulting in lower melting points.
Ionic compounds generally have a higher volatility compared to covalent compounds. This is because ionic compounds have weaker intermolecular forces that allow them to break apart and vaporize more easily at lower temperatures. Covalent compounds tend to have stronger intermolecular forces, making them less likely to evaporate at the same rate.
Melting points of covalent compounds are generally lower than those of ionic compounds. This is because covalent compounds have weaker intermolecular forces compared to the strong electrostatic forces present in ionic compounds, so they require less energy to break apart the molecules.
Ionic compounds are mad by ionic bonding The two parts of the compound ther for become one by means of moving electronioc and beoming stable there fore the bond and the compound is stronger that conalent compounds which just share the electrons needed for the two (or more ) elements to become a compound so they are weaker
there is no anwer to this question, or there is too many answers!!
Ionic compounds are generally brittle because the ionic bonds within them are strong and rigid. When a force is applied, the layers of ions in the crystal lattice can shift and become misaligned, causing the structure to break instead of bending.
In general, ionic compounds tend to have higher boiling points compared to polar covalent compounds. This is because ionic compounds have strong electrostatic forces of attraction between positively and negatively charged ions, requiring more energy to break those bonds compared to the intermolecular forces found in polar covalent compounds.
Ionic compounds have strong electrostatic forces of attraction between oppositely charged ions, which require more energy to overcome compared to the weaker intermolecular forces in molecular compounds. This results in higher melting points for ionic compounds.